Identify the correct order of standard enthalpy of formation of sodium halides :

Lattice energy is directly proportional to the charges of the ions and inversely proportional to the sum of their radii: <br/><br/> Lattice energy ∝ (Q₁Q₂) / (r₁ + r₂) <br/><br/> As we move down the group, the size of the halide ions increases, resulting in a decrease in lattice energy. This leads to a decrease in the exothermicity of the lattice energy release during the formation of sodium halides. <br/><br/> Thus, the correct order of standard enthalpy of formation of sodium halides, considering both lattice energy and electron affinity, is: <br/><br/> $\mathrm{NaF}>\mathrm{NaCl}>\mathrm{NaBr}>\mathrm{NaI}$